we will need to set up the ratio and finding the concentration of HCI. Procedure: • Grab 4 different beakers. • Add a small amount of sodium carbonate onto a weighted beaker. • For each beaker pour 10 mL‚ 15 mL‚ 20 mL‚ and 30 mL of solution A. • Add a drop or 2 of indicator to each beaker. The indicator should be Phenolphthalein. • Slowly add small amount of sodium carbonate to each one until it
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tums. HYPOTHESIS: Tums is more effective in treating heartburns that Andrews salts when used. AIM: To determine the effectiveness of Calcium Carbonate and Sodium Carbonate when used to treat heartburns. APPARATUS: Measuring Cylinder‚ Beakers‚ Spatula‚ Conical Flask‚ Measuring Scale‚ Funnel‚ Dilute HCL‚ Calcium Carbonate (Present in Tums)‚ Sodium Carbonate (Present in Andrews Salts)‚ Petri Dish‚ Rubber Stopper‚ Gas Syringe METHOD: 1. Wash all apparatus. 2. Measure and transfer
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between sodium thiosulphate (thio) and hydrochloric acid. Hydrochloric Acid + Sodium Thiosulphate "" sodium chloride + water + sulphur The reactants are both colourless‚ but one of the products‚ sulphur‚ is yellow‚ so we can use this fact to follow the rates of reaction. I am going to investigate how the concentration of the acid effects the speed of the reaction. Apparatus 1 small measuring cylinder 1 large measuring cylinder 1 small beaker 1 large beaker Hydrochloric Acid Sodium Thiosulphate
Free Chemical reaction Chlorine Sodium chloride
K+ = Violet (Can be masked by Na+) - Ca+ = Brick Red - H4N+ = no color Cobaltnitrite test for K+: -Heat NH4+ off -In a small test tube/vial‚ or spot plate and place 10-15 drops of solution to test -Then add a drop of 6M HAc and 2-3 drops of sodium cobaltnitrite reagent -Observe - ppt forms = K+ and/or H4N+ - no ppt = No K+ or H4N+ Blue Litmus test for H4N+: -Mix the sample in DIW -Add 6M NaOH -Suspend damp red litmus -Observe - red litmus turns blue = H4N+ pH test: -Test sample
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glass Crucible tongs Spatula Balance Meeker burner Ring stand Iron ring Wire gauze Forceps Sulfur Iron filings Sodium Bicarbonate Sodium Chloride Sugar Sand Magnesium ribbon Hydrochloric Acid Distilled water Filter paper 9 disposable dishes Procedure: 1. Label 7 of the dishes with the names of the following products: Sulfur‚ Iron‚ Sodium Bicarbonate‚ Sodium Chloride‚ Sugar‚ Sand‚ and Magnesium. Place small samples of each in the appropriate dishes. 2. Examine each sample with
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magnesium and calcium ions in a water sample. This was used because of the fact that these ions combine with soap molecules in water making it ‘hard’ to get sudsy; consequently the soap will not clean effectively. When water containing calcium and bicarbonate ions is heated‚ some carbon dioxide is given off. As a result‚ the solution becomes less acidic and insoluble calcium carbonate is formed: Ca2+ (aq) + 2HCO3- (aq) → CaCO3 (s) + H2O (l) +CO2 (g) Hardness of water is normally expressed as parts
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14: ------------------------------------------------- To determine the enthalpy change of reaction for: ------------------------------------------------- Na2CO3(aq) + H2O(l) + CO2(g) → 2NaHCO3(aq) Given: S1— Anhydrous sodium carbonate (Na2CO3) S2— Anhydrous sodium hydrogen carbonate (NaHCO3) A1—Aqueous sulfuric acid (H2SO4)‚ 0.500mol dm-3 Apparatus | Uncertainty | Measuring cylinder | ± 0.5 ml | Electronic Balance | ± 0.001 g | Data logger | ±0.2 ℃ | Data Collection: S1
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It can be a pure compound of sodium carbonate‚ sodium bicarbonate or sodium hydroxide or the mixture of the three with compatible percent compositions. These compositions are determined by acid-base titrations‚ a volumetric process in determining the concentration of a substance in a certain solution which uses a base or acid as the titrant. The reaction between sodium carbonate and hydrochloric acid occurs in 2 stages‚ with the formation of bicarbonate ion as the intermediate product
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Chemical #1 (4 drops) Chemical #2 (4 drops) Observations: Chemical Change (Y/N) A1 NaHCO3 Sodium Bicarbonate HCl Hydrochloric Acid A2 NaOCl Sodium Hypochlorite KI Potassium Iodide Observation 1: + Add 2 drops of starch Observation 2: A3 KI Potassium Iodide Pb(NO3)2 Lead Nitrate A4 NaOH Sodium Hydroxide C20H14O4 Phenolphthalein A5 HCl Hydrochloric Acid C20H14O4 Phenolphthalein A6 NaOH Sodium Hydroxide AgNO3 Silver Nitrate B1 AgNO3 Silver Nitrate NH4OH Aqueous Ammonia Observation 1:
Free Chemical reaction Hydrochloric acid Sodium bicarbonate
the volume of the base Cb = the concentration of the base Va = the volume of the acid Ca = the concentration of the acid n = the mole factor In the case of hydrochloric acid and Sodium Bicarbonate (Baking
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